Equimolar solutions of the following compound | vedclass

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(A) Metal halides undergo hydrolysis in water to form their corresponding hydroxides and hydrochloric acid $(HCl)$.The acidity of the resulting soluti

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$BeCl_2$

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(A) Metal halides undergo hydrolysis in water to form their corresponding hydroxides and hydrochloric acid $(HCl)$.The acidity of the resulting solution depends on the nature of the metal hydroxide formed.As we move down the group in the periodic table,the basic strength of the metal hydroxides increases due to the increase in atomic size and the decrease in ionization energy,which weakens the $M-OH$ bond.$Be(OH)_2$ is amphoteric in nature,while $Mg(OH)_2$,$Ca(OH)_2$,and $Sr(OH)_2$ are basic.Since $BeCl_2$ produces the least basic (or amphoteric) hydroxide,the solution containing $BeCl_2$ will have the highest concentration of $H^+$ ions due to the hydrolysis of the $Be^{2+}$ ion,resulting in the lowest $pH$ value.

Equimolar solutions of the following compounds are prepared separately in water. Which will have the lowest $pH$ value?

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